what is the strongest acid here?

H2SO3
H2SO4
H2SeO3
H2SeO4

For oxyacids, the acidity increases with increasing number of oxygen atoms; therefore, H2SO3 and H2SeO3 will be weaker than either H2SO4 or H2SeO4. We have a problem determining which is the stronger of H2SO4 or H2SeO4. Atoms that are larger tend to have larger acid strengths and those with increasing electronegativity of the central atom tend to be less acidic. Se is slightly larger but both have about the same electronegativity. Does your text and/or your notes list ionization constants. If so, look them up. Both acids are strong acids; therefore, their first ionization is 100% so k1 will not be listed. But k2 is a weak acid (not ionized 100%) but is still relatively large as K2s go. I looked up k2 for H2SO4 and H2SeO4 and both are listed at 1.2E-2.

So, the answer is that both are equally strong.

The strongest acid among the given options is H2SO4 (sulfuric acid). These oxyacids have a trend where acidity increases with an increasing number of oxygen atoms. Therefore, H2SO3 and H2SeO3 will be weaker acids compared to H2SO4 and H2SeO4.

To determine whether H2SO4 or H2SeO4 is stronger, we can look at ionization constants. However, in this case, both acids are strong acids, meaning their first ionization is 100% and is not listed in the ionization constants. However, the second ionization constant (k2), which represents the ionization of the second hydrogen ion, is listed.

Upon looking up the ionization constants, it is found that both H2SO4 and H2SeO4 have a k2 value of 1.2E-2. Since they have relatively identical values, we cannot definitively determine which acid is stronger based solely on this information.

To determine which acid is stronger between H2SO4 and H2SeO4, you can check their ionization constants. The ionization constant, also known as the equilibrium constant, tells us the extent to which a weak acid dissociates into ions in water.

In this case, the first ionization constant (k1) is not listed for either H2SO4 or H2SeO4 since they are both strong acids. Strong acids fully dissociate in water, so their first ionization is 100%.

However, the second ionization constant (k2) for H2SO4 and H2SeO4 is listed. Although k2 is for a weaker acid than k1, it can still give us an idea of the acid strength. The higher the value of k2, the stronger the acid.

By looking up the ionization constants, it is found that the k2 value for both H2SO4 and H2SeO4 is 1.2E-2 (1.2 x 10^-2).

Based on this information, it can be concluded that both H2SO4 and H2SeO4 are strong acids with similar acid strengths.